Answer:
Metals tend to lose electrons and non-metals tend to gain electrons, so in reactions involving these two groups, there is electron transfer from the metal to the non-metal. The metal is oxidized and the non-metal is reduced. An example of this is the reaction between the metal, sodium, and the non-metal, chlorine.
Ionic bonds form between metals and non-metals. Metals are the elements on the left side of the Periodic Table. The most metallic elements are Cesium and Francium. Metals tend to lose electrons to attain Noble Gas electron configuration. Groups 1 and 2 (the active metals) lose 1 and 2 valence electrons, respectively, because of their low Ionization energies. Non-metals are limited to the elements in the upper right hand corner of the Periodic Table. The most non-metallic element is fluorine. Non-metals tend to gain electrons to attain Noble Gas configurations. The have relatively high Electron affinities and high Ionization energies. Metals tend to lose electrons and non-metals tend to gain electrons, so in reactions involving these two groups, there is electron transfer from the metal to the non-metal. The metal is oxidized and the non-metal is reduced. An example of this is the reaction between the metal, sodium, and the non-metal, chlorine. The sodium atom gives up an electron to form the Na+ ion and the chorine molecule gains electrons to form 2 Cl- ions. The charges on these anions and cations are stabilized by forming a crystal lattice, in which each of the ions is surrounded by counter ions.
Because the left side of the periodic table contains Metals while the right side non metals. Metals gives out electrons which ALWAYS have negative charge so when they lose them, the element become more positive. Non metals accept them which make them “negative”.
Explanation:
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